chemistry curriculum map timeframe unit/concepts … · uncertainty (accuracy and precision)...

Chemistry Curriculum Map

1

Timeframe Unit/Concepts

Eligible Content Assessments Suggested Resources

Marking Periods

1 & 2

Chemistry Introduction and Problem Solving using the Scientific Method Approach

Observations Hypothesis Experiment Control Theory Law

CHEM.A.1.1.2: Classify observations as

qualitative and/or quantitative. CHEM.A.1.1.1: Classify physical or

chemical changes within a system in terms of matter and/or energy. CHEM3.2.10A6: Compare and contrast scientific theories, identify questions and concerns that guide scientific investigation, and know that both direct and indirect observations are used by scientists to study the natural world and universe. Formulate and revise explanations and models using logic and evidence. Recognize and analyze alternative explanations and models.

Labs Quizzes Unit Exam

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2

Measurements and Calculations

Scientific Notation Units (English, Metric SI) Measurements (Length, Volume Mass) Uncertainty (Accuracy and Precision) Significant Figures (Rounding Calculations) Dimensional Analysis Problem Solving Temperature conversions ( K, oC, oF) Density determinations

Matter Composition Atomic Nature Elements Compounds Molecules States of Matter (solid, liquid, gas) Matter Characteristics Physical Properties and Changes

CHEM.A.1.1.3: Utilize significant figures

to communicate the uncertainty in a quantitative observation. CHEM.A.1.2.4: Describe various ways

that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume). CHEM.A.1.1.2: Classify observations as

qualitative and/or quantitative. CHEM.A.1.1.1: Classify physical or

chemical changes within a system in terms of matter and/or energy. CHEM.A.1.2.1: Compare properties of

solutions containing ionic or molecular solutes (e.g., dissolving, dissociating).

Labs Metric Maze Quizzes Unit Exam Labs Separation Challenge Quizzes Unit Exam

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3

Chemical Properties and Changes Pure Substances Diatomic molecules Allotropes Mixtures: Homogeneous (solutions, solute, And solvent) Heterogeneous (suspension, colloid) Alloys Separation Techniques (distillation, filtration, density differences, chromatography, crystallization, charcoal absorption, decanting)

CHEM.A.1.2.2: Differentiate between

homogeneous and heterogeneous mixtures (e.g., how such mixtures can be separated).

CHEM.A.1.1.4: Relate the physical

properties of matter to its atomic or molecular structure CHEM.A.1.2.3: Describe how factors

(e.g., temperature, concentration, surface area) can affect solubility. CHEM.A.1.2.4: Describe various ways

that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume). CHEM.A.1.2.5: Describe how chemical

bonding can affect whether a substance dissolves in a given liquid.


4

Chemical Foundations Elements and Symbols Dalton’s Atomic Theory and its implications The Law of Constant Composition The Law of Definite Proportions The Law of Conservation of Matter Thomson’s Experiments Cathode Ray Plum Pudding Model Rutherford’s Experiments Alpha Scattering The Gold Foil Experiment The Structure of the Atom Protons, Neutrons, Electrons, Nucleus, Electron Cloud The Bohr Model Modern Atomic Theory Atoms and Molecules The Periodic Table *Families: Alkali, Alkaline Earth, Transition Metal, Inner Transition Metal, Halogens, Noble Gas, Hydrogen, Chalcogen, Metals, NonMetals, SemiMetals. *Trends: Ionization Energy, Atomic Radius, Electron Affinity, Boiling/Melting Points, Periodic Law *Discovery: Mendeleev, Moseley Atomic Mass Atomic Number Isotopes Ions: Cation, Anions, Prediction Charges Ionic Compounds: Forming, Subscripts,


properties of matter to its atomic or molecular structure CHEM.B.1.3.1: Explain how atoms

combine to form compounds through ionic and covalent bonding. CHEM.B.1.2.2: Apply the law of definite

proportions to the classification of elements and compounds as pure substances CHEM.A.1.2.1: Compare properties of

solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.2.1.2: Differentiate between the

mass number of an isotope and the average atomic mass of an element. CHEM.A.2.3.1: Explain how the

periodicity of chemical properties led to the arrangement of elements on the periodic table. CHEM.A.2.2.2: Predict characteristics of

an atom or an ion based on its location on the periodic table (e.g., number of valence electrons, potential types of bonds, reactivity).

Labs Family Project Quizzes Unit Exam

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5

Formula Writing, Characteristics Molecular Compounds: Identifying, Formula Writing, Characteristics

CHEM.A.2.3.2: Compare and/or predict

the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends. CHEM.A.2.1.1: Describe the evolution of

atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.B.1.2.3: Relate the percent

composition and mass of each element present in a compound.

CHEM.B.1.2.1: Determine the empirical and molecular formulas of compounds.


6

Nomenclature Naming Compounds: Metal/Nonmetal Transition Metal/ NonMetal Metal/ Polyatomic Ion Nonmetal/Nonmetal Polyatomic Ions, Oxyanions Acids Formulas From Names

CHEM.A.1.1.5: Apply a systematic set of

rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions). CHEM.A.1.2.1: Compare properties of

solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.2.3.1: Explain how the

periodicity of chemical properties led to the arrangement of elements on the periodic table. CHEM.A.2.3.2: Compare and/or predict

the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends.

Labs Practice with dice Quizzes Unit Exams

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7

Chemical Composition Counting by Weighing Average Atomic Mass Formula Weight The Mole Concept, Avogadro’s Number Molar Mass Conversions: Mole/Mole, Mole/Mass, Mole/Particle, Mole/Volume, Mass/Particle, Mass/Volume. Percent Composition Calculations Mass Percent Compound Formulas Calculating Empirical Formulas Calculating Molecular Formulas

CHEM.B.1.1.1: Apply the mole concept to

representative particles (e.g., counting, determining mass of atoms, ions, molecules, and/or formula units). CHEM.B.2.2.2: Predict the amounts of

reactants and products involved in a chemical reaction using molar volume of a gas at STP. CHEM.A.1.1.3: Utilize significant figures

to communicate the uncertainty in a quantitative observation. CHEM.A.1.1.5: Apply a systematic set of

rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions). CHEM.A.1.2.4: Describe various ways

that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume). CHEM.B.1.2.1: Determine the empirical

and molecular formulas of compounds


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8

Marking Periods 3 & 4

Chemical Reactions

Chemical Reaction Evidence of a Chemical Reaction Chemical Equation: Reactants and Products Law of Conservation of Matter Balancing Chemical Equations Physical States Coefficients


properties of matter to its atomic or molecular structure CHEM.B.2.1.5: Balance chemical

equations by applying the Law of Conservation of Matter. CHEM.A.1.2.5: Describe how chemical

bonding can affect whether a substance dissolves in a given liquid. CHEM.A.1.1.5: Apply a systematic set of

rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions). CHEM.A.2.3.2: Compare and/or predict

the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends. CHEM.A.2.3.1: Explain how the

periodicity of chemical properties led to the arrangement of elements on the periodic table.


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9

Reactions and Aqueous Solutions

Understanding the Importance of Water as a Solvent Water, a Polar Molecule Electrolytes: Strong, Weak, Non Predicting Reactions Classifying Reactions: 5 basic types Synthesis or Direct Combination Decomposition Single Replacement Double Replacement Combustion

Precipitate Reactions: Double Replacement Soluble vs Insoluble Solubility Rules Complete Molecular Equation Complete Ionic Equation Net Ionic Equation Spectator Ions Reduction/Oxidation Reactions Synthesis, Single Replacement, Decomposition Half Reactions Electrochemistry

CHEM.A.1.2.3: Describe how factors

(e.g., temperature, concentration, surface area) can affect solubility. CHEM.A.1.1.4: Relate the physical

properties of matter to its atomic or molecular structure CHEM.B.1.3.1: Explain how atoms

combine to form compounds through ionic and covalent bonding. CHEM.B.2.1.3: Classify reactions as

synthesis, decomposition, single replacement, double replacement, or combustion. CHEM.B.2.1.4: Predict products of simple

chemical reactions (e.g., synthesis, decomposition, single replacement, double replacement, combustion). CHEM.A.1.2.5: Describe how chemical


Labs Quizzes Stiochiometry Project Unit Exam

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10

Acid Base Reactions Double Replacement Reactions, Acid and Base strength Neutralization Reactions Salt

CHEM.A.1.2.1: Compare properties of

solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.1.1.5: Apply a systematic set of

rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions). CHEM.A.2.3.2: Compare and/or predict

the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends. CHEM.B.2.1.5: Balance chemical

equations by applying the Law of Conservation of Matter


11

Chemical Quantities

The Chemical Equation Molecular Information Mass Information Stiochiometry Mole/Mole Relationships Meaning of Coefficients Mole Ratio Mass Relationships Mass Calculations from a Balanced Eqn. . The Concept of Limiting Reactant Calculations involving Limiting Reactant and Excess Reactant. Calculations involved in Percent Yield.

CHEM.B.2.1.2: Use stoichiometric

relationships to calculate the amounts of reactants and products involved in a chemical reaction. CHEM.B.2.1.1: Describe the roles of

limiting and excess reactants in chemical reactions. CHEM.A.1.1.3: Utilize significant figures

to communicate the uncertainty in a quantitative observation. CHEM.A.1.2.4: Describe various ways

that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume). CHEM.B.2.2.2: Predict the amounts of

reactants and products involved in a chemical reaction using molar volume of a gas at STP.




12

Energy Properties of Energy Concepts of Temperature and Heat Exothermic and Endothermic Processes Thermodynamics Measuring Energy Changes ThermoChemistry (Enthalpy) Hess Law Entropy Energy as a Driving Force Energy and Light Emission of Energy by Atoms The Wave Mechanical Model and its development from the Bohr model Quantized Energy Electronic Configuration Electronic Configuration as it relates to the Periodic Table. Periodic Table Trends Chemical bonding Ionic Bonding Covalent Bonding Lewis Structures VSEPR model

CHEM.A.2.2.1: Predict the ground state

electronic configuration and/or orbital diagram for a given atom or ion. CHEM.A.2.2.2: Predict characteristics of

an atom or an ion based on its location on the periodic table (e.g., number of valence electrons, potential types of bonds, reactivity). CHEM.A.2.2.4: Relate the existence of

quantized energy levels to atomic emission spectra CHEM.B.1.4.2: Utilize Lewis dot

structures to predict the structure and bonding in simple compounds CHEM.B.1.4.1: Recognize and describe

different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models, ball‐and‐stick models, graphical

models, solid‐sphere models, structural

formulas, skeletal formulas, Lewis dot structures). CHEM.B.1.3.3: Use illustrations to predict

the polarity of a molecule.

Labs Computer Lab (2) Quizzes Unit Exam

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13

CHEM.B.1.3.2: Classify a bond as being

polar covalent, non‐polar covalent, or

ionic CHEM.A.2.3.2: Compare and/or predict

the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends. CHEM.A.2.3.1: Explain how the

periodicity of chemical properties led to the arrangement of elements on the periodic table. CHEM.A.2.2.3: Explain the relationship

between the electron configuration and the atomic structure of a given atom or ion (e.g., energy levels and/or orbitals with electrons, distribution of electrons in orbitals, shapes of orbitals). CHEM.A.1.1.4: Relate the physical

properties of matter to its atomic or molecular structure CHEM.A.1.2.5: Describe how chemical

bonding can affect whether a substance dissolves in a given liquid. CHEM.B.2.1.2: Use stoichiometric

relationships to calculate the amounts of reactants and products involved in a chemical reaction.


14

Gases Understand Atmospheric Pressure Gas Laws: Boyles Law: Being able to relate pressure and volume. Charles Law: Being able to relate Volume and Temperature Avogadros Law: Being able to relate volume and Moles Guy-Lussacs Law: Being able to relate Pressure and Temperature The Combined Gas Law The Ideal Gas Law Daltons Law of Partial Pressure The Kinetic Molecular Theory of Gases and its implications. Real Gases (Non-Ideal) Gas Stoichiometry


(e.g., temperature, concentration, surface area) can affect solubility. CHEM.A.1.1.3: Utilize significant figures

to communicate the uncertainty in a quantitative observation. CHEM.B.2.2.1: Utilize mathematical

relationships to predict changes in the number of particles, the temperature, the pressure, and the volume in a gaseous system (i.e., Boyle’s law, Charles’s law, Dalton’s law of partial pressures, the combined gas law, and the ideal gas law). CHEM.B.2.2.2: Predict the amounts of

reactants and products involved in a chemical reaction using molar volume of a gas at STP. CHEM.A.1.1.4: Relate the physical

properties of matter to its atomic or molecular structure CHEM.A.1.2.4: Describe various ways

that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume).

Labs Computer Lab (3) Quizzes Unit Exam



15

Liquids and Solids Intermolecular Forces: Di-pole attractions, hydrogen bonding, London Dispersion forces. Energy and Change of State Heat of Fusion Heat of Vaporization Phase Diagrams

Solutions

CHEM.B.2.1.2: Use stoichiometric

relationships to calculate the amounts of reactants and products involved in a chemical reaction. CHEM.A.1.2.3: Describe how factors

(e.g., temperature, concentration, surface area) can affect solubility. CHEM.A.1.1.4: Relate the physical


bonding can affect whether a substance dissolves in a given liquid. CHEM.A.1.2.1: Compare properties of

solutions containing ionic or molecular solutes (e.g., dissolving, dissociating).




16

Solubility The Process of dissolving Solubility Curve Concentration Mass Percent Molarity Normality Dilution Factors affecting Dissolution Solution Stoichiometry

CHEM.A.1.1.3: Utilize significant figures

to communicate the uncertainty in a quantitative observation. CHEM.A.1.2.5: Describe how chemical

bonding can affect whether a substance dissolves in a given liquid. CHEM.A.1.2.4: Describe various ways

that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume). CHEM.A.1.2.3: Describe how factors

(e.g., temperature, concentration, surface area) can affect solubility. CHEM.A.1.2.1: Compare properties of

solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.1.1.4: Relate the physical

properties of matter to its atomic or molecular structure




17

Equilibrium/Kinetics The Collision Model Conditions that Affect Reaction Rates: Concentration Temperature Nature of the Reactants State of Matter Catalyst/Inhibitor Reaction Pathway Graphs Activation Energy Activated Complex Transition State Intermediates Mechanisms Chemical Equilibrium Keq, Q Le Chateliers Principal


(e.g., temperature, concentration, surface area) can affect solubility CHEM.A.1.1.4: Relate the physical



Labs Demonstrations Quizzes Unit Exam



18

Nuclear Chemistry Introduction

Radio Active Decay Nuclear Transformations Alpha, Beta Gamma, Positron Particles Half-Life Fission Fusion Radiation Effects

Organic Chemistry Introduction

Carbon Bonding Alkanes Alkenes Alkynes Functional Groups

CHEM.B.1.4.1: Recognize and describe


models, solid‐sphere models, structural formulas, skeletal formulas, Lewis dot structures) CHEM.B.2.1.5: Balance chemical

equations by applying the Law of Conservation of Matter. CHEM.B.1.4.1: Recognize and describe


models, solid‐sphere models, structural

formulas, skeletal formulas, Lewis dot structures). CHEM.A.1.1.5: Apply a systematic set of

rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions.

Labs Quizzes Unit Exams Labs Quizzes Unit Exam

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chemistry curriculum map timeframe unit/concepts … · uncertainty (accuracy and precision)...

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